...﻿ SulfuricAcid (H2SO4)
Sulfuricacid is found in common household products such as lead-acid car batteries, detergent and fertilizers. Sulfuricacid is used in car batteries as an electrolyte in the battery plate to allow electrons to pass through. Sulfuricacid is used to make phosphoric acid, which is found in phosphate fertilizers to improve plant growth, and phosphoric acid is used to make trisodium phosphate, which is found in detergent (Want To Know It, November 8, 2011).
Physical and Chemical properties
Sulfuricacid is and oily, viscous, odorless, and dark brown to colorless liquid. It has a boiling point of 315 to 338 degrees Celsius and a melting point of 10.35 degrees Celsius. Sulfuricacid burns through organic materials to create carbon such as wood, starch, sugar, paper, and more. Sulfuricacid reacts with metals and is combustible when it contacts nitrates, carbides, chlorates, etc. Sulfuricacid is soluble in water and in ethyl alcohol.
Health Effects
Sulfuricacid is highly corrosive and can cause up to 3rd degree burns when in contact with skin, and can cause blindness when in contact with eyes. If sulfuricacid emits a mist, it may...

...Observing a Single Chemical Reaction
Qualitative vs. Quantitative Observations
Abstract:
The purpose of this experiment is to help you sharpen your observational skills. The aluminum foil was found to rust in the water containing the dissolved Copper Chloride (CuCl₂) crystals. The results of the experiments were determined through close examination and observation of both qualitative and quantitative elements of the changes that occurred when a blue crystal, Copper Chloride, reacted with aluminum foil. In conclusion, aluminum foil is turned into copper when in contact with Copper Chloride (CuCl₂) granules.
Group Members and Contributions:
Priyanka Potdar and Evani Shah both contributed equally to the final lab report of the “Observing a Single Chemical Reaction” lab. They both split up the work and eventually edited the final lab report together on Google Documents. Evani completed the Title Page and Abstract, while Priyanka completed the Discussion questions. They organized their “Observation/Data” section individually. Priyanka and Evani emailed each other for doubts and concerns, finishing their lab report on August 30, 2011
Discussion:
1. From your list of observations, select two that are clearly qualitative and explain why.
There were two clearly qualitative observations in Step 2 of the experiment. First, the Copper chloride (CuCl₂) granules were flaky substances. Second, the aluminum foil...

...﻿Experiment 6
Preparation and reactions of boric acid
Objectives:
To prepare boric acid from sodium tetraborate (borax)
To carry out tests on the prepared sample of boric acid
To study the physical and chemical properties of boric acid
Introduction:
Boron is an element in the p-block of the periodic table. It has the electron configuration of 1s22s22p1 and is in group 3 or goup 13 (IUPAC classification). In nature, it consists of two isotopes 10B (19.6%) and 11B (80.4%).
Boron is bonded to the oxygen in nature. The important sources of Boron are borax and kernite. Boron oxides and their derivatives are technologically important and are relatively inexpensive to produce. Boron oxides is very difficult to crystallise and normally exists in a glassy state (d=1.83gcm-1). Molten boron oxide has a high melting point of 450 degree celcius that is readily dissolves metal oxides to form coloured borate glasses as one of the main commercial uses of boric oxide. Particularly, borosilicate glasses find wide applications in glassblowing and the production of glass objects.
On top of the boric acid, it is also known as hydrogen borate as a weak monobasic Lewis acid. At room temperature, it exists as white powder or colourless crystals with a chemical formula of H3BO3 or B(OH)3.
Apparatus and materials:
•Sodium tetraborate
•Concentrated hydrochloric acid...

...Abstract:
The objective of the experiment was to recover pure copper through a series of transformations. A series of chemical reactions are used to purify the copper. In the end 84 percent of the original copper was left, this means that when decanting and transferring some copper was lost.
Introduction:
Stoichiometry is known as the calculation of the quantities of reactants and products in a chemical reaction and in this lab one is trying to obtain the mass of copper after a series of transformations. In this experiment separation and purification are necessary to gain a product. Some ways this is done include precipitation (The process of separating a substance from a solution as a solid.), filtration (Passing a liquid through a filter to trap unwanted particles.), decantation (To pour off without disturbing the sediment.), extraction (To obtain from a substance by chemical or mechanical action, as by pressure, distillation, or evaporation.), and sublimation (To cause (a solid or gas) to change state without becoming a liquid.). Due to the law of conservation of mass one knows that the reactants are not destroyed and no new materials are created, therefore if any mass is lost it is due to human error.
Experimental:
A piece of copper wire with a mass of 0.098 grams was obtained. The sample was dissolved in 1 mL of concentrated nitric acid (HNO3). Next 100 mL of distilled water was added in the hood to dilute the...

...Aim:
To compare the reactivity of various metals by observing their reaction with hydrochloric acid.
Materials:
2 M hydrochloric acid
Detergent
Test tubes and test tube rack
0.5 pieces of magnesium, aluminium, iron, zinc and cooper
Sand paper
Ruler
Timer
Bench mat
Method:
‎1. The surface of the magnesium was cleaned with a piece of sandpaper
2. The Magnesium was placed into a test tube
3. Three Drops of detergent were added to the test tube
4. 2cm of hydrochloric acid was added to the test tube
5. The timer was set to 5 minutes
6. Observations were recorded, including the height of foam, in a table
7. The process was repeated for the remaining metals
Hypothesis:
It was predicted that Magnesium would be most reactive metal in the experiment.
Background:
As the group number decreases, reactivity increases. As the period increases, the most reactive is towards the bottom. The alkali metals (Group 1 metals) are identified as the most reactive of all present elements on the periodic table. Seeing as potassium and sodium are both found in group 1, this will suggest that potassium will be the most reactive metal. Additionally, potassium should be more reactive than sodium as its single valence electron is placed more distant from the nucleus than sodium, meaning less energy is needed to remove the valence electron, therefore meaning the reactivity is higher.
Independent variable:
The...

...Experiment 28: The reaction of Butanols with Hydrobromic Acid
Pre-lab
Objective:
The objective of this experiment is to synthesize 1-bromobutane and 2-bromobutane with different catalyst:substrate ratios to determine which ratio is the most economically favorable.
Discussion:
In this experiment, 1-butanol or 2-butanol will be converted to the corresponding alkyl bromide with HBR, while using sulfuricacid as a catalyst. The sulfuricacid will accelerate the chemical reaction with being consumed in the process, it will increase the concentration of the protonated alcohol, which then can form an alkyl bromide by either an SN1 or SN2 reaction.
The reaction for both mechanisms depends on the concentration of protonated alcohol and the catalyst should increase the rate of the reaction. This could increase the amount of alkyl bromide produced, but it could increase the side reactions as well which would reduce product yield. Therefore this experiment will test different ratios to determine the best cost ratio.
Procedure:
Reaction:
1. Assemble an apparatus for heating under reflux using a 50-mL round-bottomed flask, a water cooled reflux condenser, and a gas trap containing 1 M NaOH. The gas trap can be omitted if you under a fume hood.
2. Weigh 72.0 mmol of your assigned alcohol...

...Identification of the Specific Heat Capacity for a Calorimeter and of the Enthalpy of an Acid-Base Reaction
Abstract
The purpose of this lab was to first, determine the specific heat capacity of a homemade calorimeter, and second, to calculate the enthalpy of reaction for an acid-base reaction between 6M KOH and 6M HNO3. To determine the specific heat capacity of the calorimeter, two differing temperatures of water were measured and volume was measured and mixed within the calorimeter. The enthalpy of reaction for an acid-base reaction was found by these steps: measure volume and the temperature for both the acid and the base; mix the acid and base within the calorimeter while recording the change in temperature with a temperature probe; and calculate the enthalpy of reaction from the data found. The specific heat capacity was found to be and average of 20.0 J/(g(°C)). The enthalpy of the reaction was found to be -64.5 kJ/mol. These values show that the specific heat of the calorimeter is nearly unimportant when calculating the enthalpy when compared to other data.
Introduction
The purposes of this experimentation was to determine the specific heat capacity constant for a homemade coffee cup calorimeter and then to investigate an acid-base reaction within the coffee...